Kinetic Theory of Gases

Flashcards covering key concepts from the Kinetic Theory of Gases, including laws, fundamental assumptions, and definitions.

Kinetic Theory of Gases

Explains the behavior of gases by assuming they are made up of tiny particles in constant random motion.

Fundamental Assumptions

Postulates that gas consists of tiny particles in constant motion, volume of individual molecules is negligible, and no intermolecular forces exist.

Perfectly Elastic Collisions

Collisions between gas molecules and container walls that do not lose kinetic energy.

Average Kinetic Energy

Directly proportional to the absolute temperature of a gas.

Boyle's Law

At constant temperature, the pressure of a fixed mass of gas is inversely proportional to its volume.

Charles' Law

At constant pressure, the volume of a fixed mass of gas is directly proportional to its absolute temperature.

Combined Gas Law

Combines Boyle’s and Charles’ laws: P₁V₁/T₁ = P₂V₂/T₂.

Ideal Gas Law

PV = nRT, describes the state of an ideal gas.

Dalton's Law of Partial Pressures

States that the total pressure of a mixture of non-reacting gases equals the sum of their partial pressures.

Gas Pressure

Due to collisions of gas particles with container walls, which increase with temperature.